The correct order of stability of the superoxides is :

{K O}_{2} > R b O_{2} > C s O_{2}

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{K O}_{2} > C s O_{2} > R b O_{2}

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C s O_{2} > R b O_{2} > {K O}_{2}

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R b O_{2} > C s O_{2} > {K O}_{2}

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Solution

The correct option is B $C s O_{2} > R b O_{2} > {K O}_{2}$
Stability of superoxides increases with increase in size and electropositivity of the metal.

The order is: $C s O_{2} > R b O_{2} > {K O}_{2}$

Hence, option $C$ is correct.

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Similar questions

Q. Assertion :The oxidation state of superoxide ion in

{K O}_{2}, {C s O}_{2}

and

{R b O}_{2}

- \frac{1}{2}

. Reason: Since the oxidation state of an alkali metal in any compound is always

+ 1

, the oxidation state of oxygen is

\frac{1}{2}

in the

O_{2}^{-}

ion.

Read the above assertion and reason and choose the correct option regarding it.

Q. The oxidation state of Na, K, Rb respectively in

N a_{2} O_{2}, K O_{2}, R b O_{2}

is :

$R b O_{2}$ is

The stability of $K_{2} O$ , $K_{2} O_{2}$ and $K O_{2}$ is in order $K_{2} O < K_{2} O_{2} < K O_{2}$ . The increasing stability at the size of metal ion increases is due to stabilization of:

Q. Potassium superoxide (

{K O}_{2}

) is used in rebreathing gas masks to generate oxygen:

{K O}_{2} (s) + H_{2} O (l) ⟶ K O H (s) + O_{2} (g)

If a reaction vessel contains 0.158 mol

{K O}_{2}

and 0.10 mol

H_{2} O

, how many moles of

O_{2}

can be produced?

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The correct order of stability of the superoxides is :

The correct option is B CsO2>RbO2>KO2Stability of superoxides increases with increase in size and electropositivity of the metal. The order is: CsO2>RbO2>KO2Hence, option C is correct.

The correct option is B $C s O_{2} > R b O_{2} > {K O}_{2}$
Stability of superoxides increases with increase in size and electropositivity of the metal.

The order is: $C s O_{2} > R b O_{2} > {K O}_{2}$

Hence, option $C$ is correct.